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selection rules and also by specific surface selection rules, differentiating various directions of the polarization of radiation and molecular orientation with respect to the surface of the electrode. Infrared reflectance spectroscopy has been used, for example, to study the structure of water in the electrical double layer, adsorption of H2 and CO on a platinum electrode and the adsorption of intermediates in the oxidation of organic substances on Pt, Au, Rh and Pd electrodes. The spectra can be interpreted in terms of the symmetry changes in the molecules in the electrochemical interface, bonding to the electrode surface, aggregation, etc. An example of the SNIFTIRS study of a Pt electrode in contact with 0.5 M LiClO4 in propylene carbonate (PC) is demonstrated in Fig. 5.35. The reference potential, E was 2 V versus Li/Li + , the working potential, w was 3.2 V versus Li/Li + . Anodic oxidation of PC is clearly apparent at these conditions; it is accompanied by the relative intensity drop of the C = O stretching vibration at 1785 cm"1 (from the intact PC), and increase of the C=O stretching vibration at 1766 cm"1 (from the oxidized PC). The oxidation products are further characterized by several new negative going peaks in the 1000-1800 cm"1 region, whereas the content of CH3 groups remains unchanged by oxidation. The most characteristic oxidation product of PC is molecular CO2 identified at 2342 cm"1. The onset of PC oxidation (CO2 formation) was detected by SNIFTIRS already at 2.1 V versus Li/Li + , which indicates that propylene carbonate is much less stable against oxidative decomposition than it was formerly believed on the basis of electrochemical methods (anodic currents at the platinum electrode in the mentioned electrolyte are practically negligible in the interval 2-4 V versus

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to form v+ cations and v_ anions and with a degree of dissociation or, we have, considering Eqs (2.4.6) and (2.4.9), K = a(U+ + U-)z+v+Fc = <x(U+ + (7_) |z_| v_Fc A = a(U+ + UJ)z+ v+F = a(U+ + UJ) |z_| v_F A* = a(U+ + UJ)F (2.4.13)

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*A:CE1# configure router static-route 0.0.0.0/0 next-hop 140.10.0.101 *A:CE1#

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The behaviour of real solutions approaches that of ideal solutions at high dilution. The molar conductivity at limiting dilution, denoted A0, is A0 = z+v+F(U + +U .) = |z_| V-F(U + + U .) = v+k + + v_A _ *o *o (2.4.14) This equation is valid for both strong and weak electrolytes, as a = 1 at the limiting dilution. The quantities A = \zt\ FU have the significance of ionic conductivities at infinite dilution. The Kohlrausch law of independent ionic conductivities holds for a solution containing an arbitrary number of ion species. At limiting dilution, all the ions conduct electric current independently; the total conductivity of the solution is the sum of the contributions of the individual ions. Because of the interionic forces, the conductivity is directly proportional to the concentration only at low concentrations. At higher concentrations, the conductivity is lower than expected from direct proportionality. This decelerated growth of the conductivity corresponds to a decrease of the molar conductivity. Figure 2.4 gives some examples of the dependence of

*B:PE1# show router route-table =============================================================== Route Table (Router: Base) =============================================================== Dest Prefix Type Proto Age Pref Next Hop[Interface Name] Metric --------------------------------------------------------------140.10.0.1/32 Local Local 02d22h03m 0 system 0 140.10.0.3/32 Remote Static 00h06m41s 5 140.10.0.102 1 140.10.0.11/32 Local Local 02d20h45m 0 loopbackTest 0 140.10.0.12/32 Remote Static 00h06m27s 5 140.10.0.102 1 140.10.0.96/30 Local Local 02d21h37m 0 toPE2 0 140.10.0.100/30 Local Local 02d21h21m 0 toCE1 0 150.10.0.0/24 Remote Static 00h57m02s 5 140.10.0.98 1 --------------------------------------------------------------No. of Routes: 7 =============================================================== *B:PE1>config>router#

Fig. 2.4 Dependence of molar conductivity of strong electrolytes on the square root of concentration c. The dashed lines demonstrate the Kohlrausch law (Eq. 2.4.15)

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